GENERAL CHEMISTRY ELECTRONIC STRUCTURE AND PERIODIC TABLE A. Electronic Structure 1. Orbital structure of hydrogen atom‚ principal quantum number n‚ number of electrons per orbital 2. Ground state‚ excited states 3. Absorption and emission spectra 4. Quantum numbers l‚ m‚ s‚ and number of electrons per orbital 5. Common names and geometric shapes for orbitals s‚ p‚ d 6. Conventional notation for electronic structure 7. Bohr atom 8. Effective nuclear
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SCH4U-C 1 UNIT Structure and Properties of Matter Unit 1 Introduction Chemisty SCH4U-C Table of Contents Unit 1: Structure and Properties of Matter Lesson 1: Atomic Structure Lesson 2: Introduction to Chemical Bonding Lesson 3: Molecular Shape and Polarity Lesson 4: Intermolecular Forces and Their Applications Unit 2: Organic Chemistry Lesson 5: Saturated Hydrocarbons Lesson 6: Unsaturated Hydrocarbons Lesson 7: Functional Groups Lesson 8: Acids‚ Esters‚ Amides
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SYLLABUS – ADVANCED PLACEMENT CHEMISTRY Required Texts 1. Chemistry: The Central Science by Brown‚ LeMay and Bursten‚ 10th ed.‚ Pearson Education. Inc.‚ Upper Saddle River‚ NJ‚ 2006‚ ISBN: 0131464892 Includes: Text book‚ Laboratory Manual‚ Student Study Guide‚ AP Test Prep Series‚ Solutions to Practice Problems 2. Barrons AP Chemistry‚ Jespersen‚ Neil D‚ 4th ed.‚ Barron’s Educational Series‚ Inc‚ 250 Wireless Boulevard‚ Hauppauge‚ New York 11788
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Max Marks: 70 Instructions: i) ii) The question paper has four parts‚ A‚ B‚ C and D. All parts are compulsory Part-A Carries 10 marks Part-B Carries 10 marks Part-C Carries 15 marks Part-D Carries 35 marks iii) Write balanced equations and draw diagrams wherever required (Use log tables and the simple commercial calculator if necessary (use of scientific calculator is not allowed) Part-A I. Answer all questions‚ 1. 2. 10 X 1=10 3. Define the term molality. How does the enthalpy change during
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This molecular orbital model can be used to explain why He2 molecules don’t exist. Combining a pair of helium atoms with 1s2 electron configurations would produce a molecule with a pair of electrons in both the bonding and the * antibonding molecular orbitals. The total energy of an He2 molecule would be essentially the same as the energy of a pair of isolated helium atoms‚ and there would be nothing to hold the helium atoms together to form a molecule. The fact that an He2 molecule is neither
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when bonds form. Lewis dot diagrams for elements are a handy way of picturing valence electrons‚ and especially‚ what electrons are available to be shared in covalent bonds. The valence electrons are written as dots surrounding the symbol for the element: one dot is place on each side first‚ and when all four positions are filled‚ the remaining dots are paired with one of the first set of dots‚ with a maximum of two dots placed on each side. Lewis-dot diagrams of the atoms in rows 1 and 2 of
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pair) into a vacant orbital of a central metal ion and so dative covalent (co-ordinate) bonds hold a complex together. The central metal ion with vacant bonding orbitals can act as a Lewis acid. Ligands act as Lewis bases by electron pair donation to form the metal-ligand bond. Bronsted-Lowry acid-base theory reminders (essentially a sub-set of Lewis Theory) A base is a proton acceptor. This is via an electron lone pair on the base (a Lewis base is a lone pair donor). e.g. NH3‚ HCO3-‚ OH- etc
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UNIT 1 MATTER‚ CHEMICAL TRENDS AND CHEMICAL BONDING UNIT 1 MATTER AND CHEMICAL BONDING 1.1 The Study of Chemistry Chemistry is the study of matter and its properties‚ the changes (chemical‚ physical‚ and nuclear) that matter experiences‚ and the energy that is associated with these changes. The term STSE refers to science‚ technology‚ society‚ and the environment. These four areas are
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∙ As n increases‚ the size of the orbital increases‚ and the electron is easier to remove. ∙ Exceptions : Be to B decrease in IE shows that the electrons in 2s orbital effectively shield the 2p electron. N to O- drop in IE because of addition of electron in first p orbital that results in a pair that repel each other and make either of them easier to remove. Electron Affinity X(g) + e-→
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short answer questions‚ most broken down into smaller parts. This is often an eclectic‚ unpredictable mix of questions from various units‚ and may demand students write short paragraphs‚ use equations and reference tables‚ or draw graphs and diagrams in order to correctly answer the questions. Students taking the exam should come with a 4-function or scientific calculator (not a graphing calculator)‚ pen‚ and pencil. Reference Tables will be provided. Students are required to stay in the examination
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